Print Options

Font size:

← Back to notecard set|Easy Notecards home page

Print this list...Print as notecards

Chem test!

1.

London dispersion forces are formed due to instantaneous ______________ formation.

dipole

2.

From these three choices, CH4 , NH3 and H2O , which one does NOT have the capacity for hydrogen bonding?

CH4 does not use hydrogen bonding because the difference in electronegativity between C and H is too small.

3.

Which statement explains the attraction between the water molecules?

Water is a polar molecule. The slightly negative end of the molecule attracts to the slightly positive end of other molecules. This forms a weak connection between the molecules.

4.

Which of the following compounds are most likely to form hydrogen bonds?

H2O

5.

Which of the following statements best explains why ice floats on water?

Hydrogen bonding causes water to be less dense in the solid state than in the liquid state .

6.

Substances that exhibit hydrogen bonding or dipole-dipole forces are generally soluble in ______________.

water

7.

Are melting points of molecular compounds generally higher than, lower than, or the same as those of ionic compounds?

lower than

8.

Which statement best explains these properties?

Ammonia is polar and experiences hydrogen bonding attractions between neighboring molecules and makes it harder to overcome the intermolecular forces needed for the phase change from liquid to gas.

9.

Intermolecular forces include all of the following EXCEPT:

covalent bonding

10.

The most important intermolecular force in CCl4 is:

london dispersion forces

11.

The ________ shape of water allows several water molecules to bond together, which influences its physical properties.

bent

12.

Select the substance with the lowest boiling point and identify the most important intermolecular force responsible for the difference in boiling point.

CH4 has the lowest boiling point because it uses London dispersion forces.

13.

London dispersion forces are formed due to instantaneous _____ formation.

dipole

14.

What is a term for attractive forces that occur between polar molecules?

dipole-dipole forces

15.

Generally, are London dispersion forces stronger or weaker than dipole-dipole forces?

weaker

16.

Movement of the ____________ creates the London dispersion forces.

electrons

17.

When you put sodium metal in liquid ammonia, what is the intermolecular attraction between Na+ ions and NH3 molecules?

Ion-dipole

18.

When KOH dissolved in ethanol, what is the intermolecular attraction between OH- ions and C2H5OH molecules?

Ion-dipole`

19.

Which statement about London dispersion forces is TRUE?

London Dispersion forces are temporary in nature.

20.

When KCl dissolved in ethanol, what is the intermolecular attraction between K+ ions and ethanol molecules?

Ion-dipole

21.

What are dipole-dipole forces?

intermolecular force between polar molecules

22.

Which noble gas below has the lowest boiling point?

Ne

23.

Which of the following is the weakest intermolecular force?

London dispersion force

24.

When KNO3 dissolved in water, what is the intermolecular attraction between NO3 - ions and H2O molecules?

Ion-dipole

25.

Which of the following statements best explains why ice floats on water?

Hydrogen bonding causes water to be less dense in the solid state than in the liquid state.

26.

Which of the following compounds is most likely to form hydrogen bonds?

H2O

27.

The _________ shape allows several water molecules to bond together, which influences its physical properties.

bent

28.

Which of the following compounds is/are most likely to form hydrogen bonds?

HF

29.

Complete the sentence using one of the following terms: proton, neutron or electron.

When H is covalently bonded to N, O or F, the strongly electronegative atoms pull the electrons in the covalent bond close to themselves, leaving H as almost a bare ___________.

proton

30.

Which of the following does not have hydrogen bonds?

Hydrogen chloride

31.

The O-H covalent bond in a water molecule is best described as being _____.

very polar

32.

In addition to hydrogen bonding, what also contributes to the fact that ice is less dense than liquid water?

its bent shape

33.

In the case of hydrogen bonds, the hydrogen donor is strongly:

Electronegative

34.

True or False:

Because the molecular weight of hydrogen chloride is heavier than that of water, the boiling point of hydrogen chloride is higher than that of water

False

35.

Properties of solids depend on:

All of the above

36.

Complete the sentence using one of the following terms: water, hexane or oil.

Substances that exhibit hydrogen bonding or dipole-dipole forces are generally soluble in __________.

water

37.

Are melting points of molecular compounds generally higher or lower than those of ionic compounds?

lower

38.

Intermolecular forces are _____ as compared to intra-molecular forces.

Much weaker

39.

What type of solid is diamond?

covalent network

40.

Why do covalent crystals have high melting and boiling points?

The network covalent bond is very strong.

41.

Which of the following statements is wrong?

Covalent compounds are generally soluble in polar solvents

42.

Diamond is composed entirely of _____ atoms that are connected by _____ bonds.

carbon; covalent

43.

Intermolecular forces include all of the following EXCEPT _____

covalent bonding

44.

Nonpolar solvents will most easily dissolve solids that are

nonpolar.

45.

This is the structure picture of fullerene (C60).

The type of chemical bond that holds fullerene (C60) together is

covalent